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2 years ago

What is the molar mass of 81.50g of gas exerting a pressure of 1.75atm on the walls of a 4.92L container at 307K?

2 answers:

7 0

M = 81.50g, mm = m/n
n = ???
PV = nRT --> n = PV/RT
n = (1.75)(4.92)/(.0821)(307)
n = 8.61/25.20 = .342
--> mm = m/n = 81.5/.342 = 238.58

algol [13]2 years ago

7 0

Answer: Molar mass of gas is 238.6 g/mol

Explanation:

Using ideal gas equation:

PV = nRT

P= pressure = 1.75 atm

V= volume = 4.92 L

n = no of moles = $\frac{\text {given mass}}{\text {Molar mass}}=\farc{81.5}{M}$

R= gas constant =0.0821 Latm\molK

T = temperature = 307 K

R= gas constant = 8.314 J/Kmol

T= temperature = 190.7 K

M= molecular mass of gas = ?g/mol

$1.75\times 4.92=\frac{81.5}{M}\times 0.0821\times 307$

$M=238.6g/mol$

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A raindrop has a mass of 50. mg and the Pacific Ocean has a mass of 7.08 x 10^20 kg. what is the mass of 1 mole of raindrops? Ho

Anna007 [38]

Solution:

According to the Avogadro's number:

6.022 *10^23 drops per 0.050 g/ drop = 3.011 *10^22 grams per mole of drops

3.011 *10^22 grams per 1 kg / 1000 grams = 3.011 *10^19 kilograms / mole of drops

thus the answers are:

3.0 *10^22 grams per mole of drops

3.0 *10^19 kilograms per mole of drops

And,

In the calculation of how many moles of raindrops in the Pacific Ocean is:

7.08X10^20kg per 3.0 *10^19 kilograms per mole of drops = 23.5 moles of drops

This is the required solution.

7 0

2 years ago

Read 2 more answers

Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°

Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

$PV = \frac{m}{M}RT$

$PxM = \frac{m}{V}RT$

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

$2.7 = \frac{0.94xMavg}{0.082x289}$

0.94Mavg = 63.9846

Mavg = 68.0687 g/mol

The molar mass of N is 14 g/mol and of O is 16 g/mol, than $M_{NO2} = 46$ g/mol and $M_{N2O4} = 96$ g/mol. Calling y the molar fraction:

$Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}$

And,

$y_{NO2} + y_{N2O4} = 1$

$y_{N2O4} = 1 - y_{NO2}$

So,

$68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})$

$68.0687 - 92 = 46y_{NO2} - 92y_{NO2}$

$46y_{NO2} = 23.9313$

$y_{NO2} = 0.52$

$y_{N2O4} = 0.48$

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

8 0

2 years ago

If the human body were a car, glucose would be:

NeTakaya

<span>If the human body were a car, glucose would be the gasoline.
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8 0

2 years ago

You are given three bottles labeled a, b, and

ElenaW [278]

Answer :Solid in bottle a is ionic, solid in bottle b is molecular and solid in bottle c is ionic.

Explanation :

Ionic compound is formed when a metal atom donates one or more electrons to a non metal. This results in the formation of a cation ( a positive ion) and an anion ( a negative ion). These ions are bonded to each other by electrostatic attraction.

The intermolecular forces in case of a an ionic compound are very strong.

The melting point of a substance depends on how strongly the molecules are attracted to each other. Stronger the forces, higher is the melting point.

Therefore ionic compounds always have very high melting points.

On the other hand, covalent compounds have weak intermolecular forces. Therefore they have low melting points.

Based on above discussion, we can classify the given compounds as follows.

a) Solid in bottle a is Ionic as it has high melting point.

b) Solid in bottle b is molecular as it has low melting point.

c) Solid in bottle c is Ionic as it has high melting point.

6 0

2 years ago

How many moles are there in 45.0 grams of sulfuric acid,<br> H2SO4?

olga2289 [7]

Answer:

the answer is 0.4588162459

Explanation:

1 mole = 0.010195916576195

= 45 ×"

5 0

2 years ago